The single-phase KZn2(PO4)(HPO4) was synthesized via solid-state reaction at 80 °C using
K3PO4·3H2O, K2HPO4·3H2O, and ZnSO4·7H2O as raw materials. The thermal decomposition of KZn2(PO4)(HPO4) experienced one step, which was the intramolecular
dehydration of the protonated phosphate groups to form Zn2P2O7. The apparent activation energy E
a was estimated with six comparative isoconversional
procedures. The average value of the apparent activation energy E
a associated with the thermal decomposition
of KZn2(PO4)(HPO4) was determined
to be 411.49 ± 14.37 kJ mol–1, which demonstrates
that the thermal decomposition of KZn2(PO4)(HPO4) is a single-step kinetic process and can be described by
a unique kinetic triplet [E
a, A, g(α)]. A new modified method for
multiple rate isotemperature was used to define the most probable
reaction mechanism g(α), and reliability of
the used method for the determination of the kinetic mechanism was
tested by the comparison between experimental plots and modeled results
for every heating rate. The results show that the mechanism function
is reliable. The value of pre-exponential factor A was obtained on the basis of E
a and g(α). Some thermodynamic functions (ΔS
⧧, ΔH
⧧, and ΔG
⧧) of the transition
state complex were also calculated.
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